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A valence electron is an electron that is associated with an atom, and that can participate in the formation of a chemical bond; in a single covalent bond, both atoms in the bond contribute one valence electron in order to form a shared pair. The presence of valence electrons can determine the element's chemical properties and whether it may bond with other elements: For a main group element, a valence electron can only be in the outermost electron shell. An atom with a closed shell of valence electrons (corresponding to an electron configuration \(s^2p^6\)) tends to be chemically inert. An atom with one or two valence electrons more than a closed shell is highly reactive, because the extra valence electrons are easily removed to form a positive ion. An atom with one or two valence electrons fewer than a closed shell is also highly reactive, because of a tendency either to gain the missing valence electrons (thereby forming a negative ion), or to share valence electrons (thereby forming a covalent bond). Like an electron in an inner shell, a valence electron has the ability to absorb or release energy in the form of a photon. An energy gain can trigger an electron to move (jump) to an outer shell; this is known as atomic excitation. Or the electron can even break free from its associated atom's valence shell; this is ionization to form a positive ion. When an electron loses energy (thereby causing a photon to be emitted), then it can move to an inner shell which is not fully occupied. The number of valence electronsThe number of valence electrons of an element can be determined by the periodic table group (vertical column) in which the element is categorized. With the exception of groups 3–12 (the transition metals), the units digit of the group number identifies how many valence electrons are associated with a neutral atom of an element listed under that particular column.  The periodic table of the chemical elements Periodic table groupValence ElectronsGroup 1 (I) (alkali metals)1Group 2 (II) (alkaline earth metals)2Groups 3-12 (transition metals)2* (The 4s shell is complete and cannot hold any more electrons)Group 13 (III) (boron group)3Group 14 (IV) (carbon group)4Group 15 (V) (pnictogens)5Group 16 (VI) (chalcogens)6Group 17 (VII) (halogens)7Group 18 (VIII or 0) (noble gases)8*** The general method for counting valence electrons is generally not useful for transition metals. Instead the modified d electron count method is used. ** Except for helium, which has only two valence electrons. The Concept of Open Valence ("Valence")The valence (or valency) of an element is a measure of its combining power with other atoms when it forms chemical compounds or molecules. The concept of valence was developed in the last half of the 19th century and was successful in explaining the molecular structure of many organic compounds. The quest for the underlying causes of valence lead to the modern theories of chemical bonding, including Lewis structures (1916), valence bond theory (1927), molecular orbitals (1928), valence shell electron pair repulsion theory (1958) and all the advanced methods of quantum chemistry. The combining power or affinity of an atom of an element was determined by the number of hydrogen atoms that it combined with. In methane, carbon has a valence of 4; in ammonia, nitrogen has a valence of 3; in water, oxygen has a valence of two; and in hydrogen chloride, chlorine has a valence of 1. Chlorine, as it has a valence of one, can be substituted for hydrogen, so phosphorus has a valence of 5 in phosphorus pentachloride, PCl5. Valence diagrams of a compound represent the connectivity of the elements, lines between two elements, sometimes called bonds, represented a saturated valency for each element.[1] Examples are:- CompoundH2CH4C3H8C2H2NH3NaCNH2SH2SO4Cl2O7DiagramHydrogen 1Carbon 4 Hydrogen 1Carbon 4 Hydrogen 1Nitrogen 3 Hydrogen 1Sodium 1 Carbon 4 Nitrogen 3Sulfur 2 Hydrogen 1Sulfur 6 Oxygen 2 Hydrogen 1Chlorine 7 Oxygen 2 Valence only describes connectivity, it does not describe the geometry of molecular compounds, or what are now known to be ionic compounds or giant covalent structures. The line between atoms does not represent a pair of electrons as it does in Lewis diagrams. Further ReadingKhan Academy Valence Electrons Cliffs Notes Valence Electrons Contributors
1.3: Valence electrons and open valences is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts. What period has 5 valence electrons?Therefore, the element in the fourth period of the periodic table which has five valence electrons is Arsenic.
What elements have 5 electrons?Atomic Number. What is the only metal with 5 valence electrons?The elements of group 15 (column) VA of the periodic table all have electron configurations of s2p3 , giving them five valence electrons. These elements include Nitrogen (N), Phosphorus (P), Arsenic (As), Antimony (Sb) and Bismuth (Bi).
Which element has 5 valence electrons B or P?Phosphorus has five valence electrons in its valence shell. The atomic number of phosphorus is 15.
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What is an element with 5 valence electrons?
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